Question

What does the given reaction indicate?
$Cu+2AgN{{O}_{3}}\to Cu{{(N{{O}_{3}})}_{2}}+2Ag$

Answer 1

First, find the oxidation number of each element in the reaction, if the oxidation number of one element increases and the oxidation number of other elements decreases in the same reaction then, we can say that it is a redox reaction.

Complete answer:
We know that reaction is a process in which certain substances, i.e., reactants react with each other to form new substances, i.e., products. When they are written in the chemical formula, it is known as a chemical equation. So, there are many types of reactions, like combination reaction, displacement reaction, double-displacement reaction, combustion reaction, redox reaction exothermic reactions, endothermic reaction, equilibrium reaction, etc.
So, the given reaction in the question is:
$Cu+2AgN{{O}_{3}}\to Cu{{(N{{O}_{3}})}_{2}}+2Ag$
We can find the oxidation number of all the elements in the reaction.
On the reactant side, the oxidation number of Cu is 0, the oxidation number of Ag in $AgN{{O}_{3}}$ is +1 and the oxidation number of the nitrate ion ($NO_{3}^{-}$) is -1. On the product side, the oxidation number of Cu in $Cu{{(N{{O}_{3}})}_{2}}$ is +2, the oxidation number of the nitrate ion ($NO_{3}^{-}$) is -1, and the oxidation number of Ag is 0.
So, Cu changes from 0 to +2, which means it is oxidized and Ag changes from +1 to 0, which means it is reduced. Therefore, in the same reaction oxidation and reduction occurs, it is a redox reaction.

Note:
It is not necessary that there must be two different elements in the reaction for the oxidation and reduction to occur, even the same reactant can undergo oxidation in one product and reduction in the other.